When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution(dissolving) can be determined using a coffee cup calorimeter.ThermometerCardboard orIn the laboratory a general chemistry student finds that when 3.38 g of CuCl,(s) areStyrofoam liddissolved in 114.10 g of water, the temperature of the solution increases from 25.37 to27.99 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant)was determined in a separate experiment to be 1.60 J/°C.NestedStyrofoam cupsBased on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) inkJ/mol.- Reactionoccurs inAssume the specific heat of the solution is equal to the specific heat of water.solution.AHdissolutionkJ/molkc Cengage Ln

Heat absorbed by calorimeter=Heat capacity of calorimeter×Temperature change…

/hen a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution lissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboan the laboratory a general chemistry student finds that when 3.38 g of CuCl2(s) are Styrofoa ssolved in 114.10 g of water, the temperature of the solution increases from 25.37 to 7.99 °C. he heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) as determined in a separate experiment to be 1.60 J/°C. Nest Styr ased on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in I/mol. Reac ocCL ssume the specific heat of the solution is equal to the specific heat of water. solu Haissolution kJ/mol

/hen a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution lissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboan the laboratory a general chemistry student finds that when 3.38 g of CuCl2(s) are Styrofoa ssolved in 114.10 g of water, the temperature of the solution increases from 25.37 to 7.99 °C. he heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) as determined in a separate experiment to be 1.60 J/°C. Nest Styr ased on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in I/mol. Reac ocCL ssume the specific heat of the solution is equal to the specific heat of water. solu Haissolution kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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